Bissoy.com
Doctors Medicines MCQs Q&A

Henry Law’s Constants at a system temperature of 25°C (77°F) of oxygen is 756.7 atm/(mol/litre). Molar Weight of O2 is 31.9988 g/mol and partial fraction in air is ~ 0.21. Calculate the Oxygen dissolved in the Water at atmospheric pressure.

Henry Law’s Constants at a system temperature of 25°C (77°F) of oxygen is 756.7 atm/(mol/litre). Molar Weight of O2 is 31.9988 g/mol and partial fraction in air is ~ 0.21. Calculate the Oxygen dissolved in the Water at atmospheric pressure. Correct Answer 0.0089 g/liter

Oxygen dissolved in the Water at atmospheric pressure can be calculated as: c = pg / kH co = (1 atm) 0.21 / (756.7 atm/(mol/litre)) (31.9988 g/mol) = 0.0089 g/liter.

Related Questions

Glucose isomerase is used extensively in the USA for production of high-fructose syrup. The reaction is ___________ Glucose ⇄ Fructose ΔH°rxn for this reaction is 5.73 kJ gmol-l; ΔS°rxn is 0.0176 kJ gmol-l K-l. Calculate the equilibrium constants at 50°C. (Given R = 8.3144J gmol-l K-l =8.3144×10-3 kJ gmol-lK-l).
The Henry’s law constant for O2 in water at 25°C is 1.27×10−3M/atm and the mole fraction of O2 in the atmosphere is 0.21. Calculate the solubility of O2 in water at 25°C at an atmospheric pressure of 1.00 atm. Strategy: ▪ Use Dalton’s law of partial pressures to calculate the partial pressure of oxygen. ▪ Use Henry’s law to calculate the solubility, expressed as the concentration of dissolved gas.
Henry Law’s Constants at a system temperature of 25°C (77°F) of nitrogen is 1600 atm/(mol/litre). Molar weight of N2 is 28.0134 g/mol and partial fraction in air is ~ 0.79. Calculate the Nitrogen dissolved in the Water at atmospheric pressure.
The atmospheric pressure is 1.0 atm and Henry’s law constant for O2 is 1.66 x 10−6 M/mm Hg at 25 °C. Assume air contains 21% oxygen. Calculate the partial pressure of oxygen. (21% of air is oxygen and the mole fraction of O2 is 0.21).
What is the condition for a tree to be weight balanced. where a is factor and n is a node? >= a*weight and weight >= a*weight. b) weight >= a*weight and weight >= a*weight. c) weight >= a*weight and weight >= a*weight. d) weight is a non zero
Oxygen diffuses through a stagnant layer of air, 1mm thick, ambient temperature 28°C and 1atm total pressure. The partial pressure of oxygen on two sides of layer is P1=0.9atm and P2=0.1atm respectively. Calculate the value of Molar flux (in mol/m2.s) with respect to an observer moving with molar average velocity. Calculate this value at the end of the path where P2=0.1atm. Use R=8.205*10-5m3atmK-1mol-1.
What is the total pressure of contained if it contains 0.5 fraction of O2 with partial pressure 3 Pa, 0.3 fraction of H2 with partial pressure 5 Pa, 0.2 fraction of CO2 with partial pressure 15 Pa?
What is the total pressure of contained if it contains 0.3 fraction of N2 with partial pressure 8 Pa, 0.3 fraction of H2 with partial pressure 2 Pa, 0.4 fraction of CO2 with partial pressure 15 Pa?
What is the fraction of a gas in a system at partial pressure 1 mm Hg, if the 0.2 fraction of the same gas is at partial pressure 2 mm Hg and 0.3 fraction at partial pressure 3 mm Hg (Use Freundlich Isotherm)?
What is the fraction of a gas in a system at partial pressure 2 mm Hg, if the 0.2 fraction of the same gas is at partial pressure 8 mm Hg and 0.3 fraction at partial pressure 18 mm Hg (Use Freundlich Isotherm)?